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Chapter 21: Electrochemistry Chemical Change and Electrical Work

Chapter 21: Electrochemistry Chemical Change and Electrical Work. 21.5 Electrochemical Processes in Batteries. Chemistry of Batteries. Dry Cells. Anode (oxidation): Zn (s) Zn 2+ (aq) + 2 e - Cathode (reduction):

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Chapter 21: Electrochemistry Chemical Change and Electrical Work

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  1. Chapter 21: Electrochemistry Chemical Change and Electrical Work 21.5 Electrochemical Processes in Batteries

  2. Chemistry of Batteries Dry Cells Anode (oxidation): Zn(s) Zn2+(aq) + 2 e- Cathode (reduction): 2 MnO2 (s) + 2 NH4+(aq) + 2 e- Mn2O3 (aq) + 2 NH3 (aq) + H2O(l) ammonia is tied up with Zn2+ Zn2+(aq) + 2 NH3 (aq) + 2 Cl-(aq) Zn(NH3)2Cl2 (s) Overall (cell) reaction: 2 MnO2 (s) + 2NH4Cl(aq) + Zn(s) Zn(NH3)2Cl2 (s) + H2O(l) +Mn2O3 (s) Ecell = 1.5 V Alkaline Battery Anode (oxidation): Zn(s) + 2 OH-(aq) ZnO(s) + H2O(l) + 2 e - Cathode (reduction): MnO2 (s) + 2 H2O(l) + 2 e - Mn(OH)2 (s) + 2 OH -(aq) Overall (cell) reaction: Zn(s) + MnO2 (s) + H2O(l) ZnO(s) + Mn(OH)2 (s)Ecell = 1.5 V

  3. Dry Cell and Alkaline Battery Gallery (p. 924)

  4. Chemistry of Batteries Mercury and Silver (Button) Batteries Anode (oxidation): Zn(s) + 2 OH-(aq) ZnO(s) + H2O(l) Cathode (reduction) (mercury): HgO(s) + H2O(l) + 2 e- Hg(l) + 2 OH-(aq) Cathode (reduction) (silver): Ag2O(s) + H2O(l) + 2 e- 2 Ag(s) + 2 OH-(aq) Overall (cell) reaction (mercury): Zn(s) + HgO(s) ZnO(s) + Hg(l); Ecell = 1.3 V Overall (cell) reaction (silver): Zn(s) + Ag2O(s) ZnO(s) + 2 Ag(s); Ecell = 1.6 V

  5. Gallery (p. 925)

  6. Chemistry of Batteries Secondary (Rechargeable) Batteries Lead-Acid Batteries Anode (oxidation): Pb(s) + SO42-(aq) PbSO4 (s) + 2 e- Cathode (reduction): PbO2 (s) + 4 H+(aq) + SO42-(aq) + 2 e- PbSO4 (s) + 2 H2O(l) Overall (cell) reaction (discharge): PbO2 (s) + Pb(s) + 2 H2SO4 (aq) 2 PbSO4 (s) + 2 H2O(l); Ecell = 2 V Overall cell) reaction (recharge): 2 PbSO4 (s) + 2 H2O(l) PbO2 (s) + Pb(s) + 2 H2SO4 (aq)

  7. Gallery (p. 925)

  8. Automotive Application: the Discharge and Recharging of a Lead-Acid Battery Fig. 21.18

  9. Chemistry of Batteries Secondary (Rechargeable) Batteries (Continued) Nickel-Cadmium (Nicad) Battery Anode (oxidation): Cd(s) + 2 OH-(aq) Cd(OH)2 (s) + 2 e- Cathode (reduction): 2 NiO(OH)(s) + 2 H2O(l) + 2 e- 2 Ni(OH)2 (s) + 2 OH-(aq) Overall (cell) reaction: Cd(s) + 2 NiO(OH)(s) + 2 H2O(l) 2 Ni(OH)2 (s) + Cd(OH)2 (s) Ecell = 1.4 V Lithium Solid-State Battery Anode (oxidation): Li(s) Li+ (in solid electrolyte) + e- Cathode (reduction): MnO2 (s) + Li+ + e- LiMnO2 (s) Overall (cell) reaction: Li(s) + MnO2 (s) LiMnO2 (s); Ecell = 3 V

  10. Lithium Solid-State Battery Nickel-Cadmium (Nicad) Battery Gallery (p. 926)

  11. Chemistry of Batteries 2 NH3 (g) + 3/2 O2 (g) N2 (g) + 3 H2O(l) N2H4 (g) + O2 (g) N2 (g) + 2 H2O (l) CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O(l) Flow Batteries (Fuel Cells) The Hydrogen Oxygen Fuel Cell Anode (oxidation): H2 (g) + CO32-(l) H2O(g) + CO2 (g) + 2 e- Cathode (reduction): 1/2 O2 (g) + CO2 (g) + 2 e- CO32-(l) Overall (cell) reaction: H2 (g) + 1/2 O2 (g) H2O(g)Ecell = 1.2 V Other Fuel Cells:

  12. Gallery (p. 926)

  13. Chemistry of Batteries Advanced Designs: Aluminum-Air Battery Anode (oxidation): 4[Al(s) + 4 OH-(aq) Al(OH)4-(aq) + 3 e-] Cathode (reduction): 3[O2 (g) + 2 H2O(l) + 4 e- 4 OH-(aq) Overall (cell) reaction: 4 Al(s) + 3 O2 (g) + 6 H2O(l) + 4 OH-(aq) 4 Al(OH)4-(aq); Ecell = 2.7 V Sodium-Sulfur Battery Anode (oxidation): 2 Na(l) 2 Na+(l) + 2 e- Cathode (reduction): n/8 S8 (l) + 2 e-nS 2-(l) Overall (cell) reaction: 2 Na(l) + n/8 S8 (l) Na2Sn (l); Ecell = 2.1 V

  14. Advanced Designs (Sodium-Sulfur Battery) Gallery (p. 927)

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